Solutions Lecture-1
Concept of solubility
Ionic \quad H-O \quad H-bonding
Anthracene → \rightarrow → Water
Non-polar \quad\quad Polar
Concept of solubility → \rightarrow → Exothermic & Endothermic reaction → \rightarrow → Vapour pressure of Liquid- Liquid solution → \rightarrow → Example → \rightarrow → Vapour pressure of solution of solid in liquid → \rightarrow → Ideal Solution & Non-Ideal Solution → \rightarrow → Azeotropes
Solutions Lecture-1
Concept of solubility
Concept of solubility → \rightarrow → Exothermic & Endothermic reaction → \rightarrow → Vapour pressure of Liquid- Liquid solution → \rightarrow → Example → \rightarrow → Vapour pressure of solution of solid in liquid → \rightarrow → Ideal Solution & Non-Ideal Solution → \rightarrow → Azeotropes
Solutions Lecture-1
Exothermic & Endothermic reaction
According to le chatelier’s principle
Δ H < 0 \Delta H<0 Δ H < 0 → \rightarrow → exothermic reaction move backward
Δ H > 0 \Delta H>0 Δ H > 0 endothermic reactionmove forward
A g A_g A g → {\rightarrow} → A l A_l A l condensation
Concept of solubility → \rightarrow → Exothermic & Endothermic reaction → \rightarrow → Vapour pressure of Liquid- Liquid solution → \rightarrow → Example → \rightarrow → Vapour pressure of solution of solid in liquid → \rightarrow → Ideal Solution & Non-Ideal Solution → \rightarrow → Azeotropes
Solutions Lecture-1
Vapour pressure of Liquid- Liquid solution
Raoult’s law:
P A ∝ x A P_A \propto x_A P A ∝ x A
P B ∝ x B P_B \propto x_B P B ∝ x B
P A P_A P A = P A 0 P_A^0 P A 0 x A x_A x A , P B P_B P B = P B 0 P_B^0 P B 0 x B x_B x B
P T P_T P T =P A P_A P A + P B P_B P B
x A = 1 , P A = P A o \ x_A=1, \quad P_A=P_A^o x A = 1 , P A = P A o
x B = 1 , P B = P B o \ x_B= 1, \quad P_B=P_B^o x B = 1 , P B = P B o
Concept of solubility → \rightarrow → Exothermic & Endothermic reaction → \rightarrow → Vapour pressure of Liquid- Liquid solution → \rightarrow → Example → \rightarrow → Vapour pressure of solution of solid in liquid → \rightarrow → Ideal Solution & Non-Ideal Solution → \rightarrow → Azeotropes
Solutions Lecture-1
Vapour pressure of Liquid- Liquid solution
Raoult’s law:
P T = P A o x A + P B o x B P_T=P^o_A x_A + P^o_B x_B P T = P A o x A + P B o x B
P T = P A o x A + P B o ( 1 − x A ) P_T=P^o_A x_A + P^o_B(1-x_A) P T = P A o x A + P B o ( 1 − x A )
P T = P B o + ( P A o − P B o ) x A P_T=P^o_B + (P^o_A - P^o_B)x_A P T = P B o + ( P A o − P B o ) x A
Concept of solubility → \rightarrow → Exothermic & Endothermic reaction → \rightarrow → Vapour pressure of Liquid- Liquid solution → \rightarrow → Example → \rightarrow → Vapour pressure of solution of solid in liquid → \rightarrow → Ideal Solution & Non-Ideal Solution → \rightarrow → Azeotropes
Solutions Lecture-1
Example
A = C H C l 3 A=CH Cl_3 A = C H C l 3 , P A o P_A^{o} P A o = 200mmHg 119.5 0.213 \quad 119.5 \quad 0.213 119.5 0.213
B = C H 2 C l 2 B = CH_2 Cl_2 B = C H 2 C l 2 ,P B o P_B^{o} P B o =415mmHg 85 g / m s 0.470 \quad 85 g/ms \quad 0.470 85 g / m s 0.470
Calculate vapour pressure of the solution prepared 25.5g C H C l 3 CH Cl_3 C H C l 3 and 40g of C H 2 C l 2 CH_2 Cl_2 C H 2 C l 2
Solution
Concept of solubility → \rightarrow → Exothermic & Endothermic reaction → \rightarrow → Vapour pressure of Liquid- Liquid solution → \rightarrow → Example → \rightarrow → Vapour pressure of solution of solid in liquid → \rightarrow → Ideal Solution & Non-Ideal Solution → \rightarrow → Azeotropes
Solutions Lecture-1
Example
x A = n A n A + n B = 0.213 0.213 + 0.478 x_A=\frac{n_A}{n_A+n_B}=\frac{0.213}{0.213+0.478} x A = n A + n B n A = 0.213 + 0.478 0.213
x B = 1 − x A x_B=1-x_A x B = 1 − x A
x A = n A n A + n B = 0.213 0.213 + 0.470 = 0.312 x_A= \frac {n_A} {n_A + n_B} =\frac {0.213} {0.213+0.470}=0.312 x A = n A + n B n A = 0.213 + 0.470 0.213 = 0.312
x B = 1 − x A = 1 − 0.312 = 0.688 x_B=1-x_A =1-0.312=0.688 x B = 1 − x A = 1 − 0.312 = 0.688
P A = x A P A 0 P_A=x_A P^0_A P A = x A P A 0 = 0.312×200=62.4 mmHg
P B P_B P B =0.688×415=285.5 mmHg
P T P_T P T = P A + P B P_A+ P_B P A + P B =347.9 mmHg
Concept of solubility → \rightarrow → Exothermic & Endothermic reaction → \rightarrow → Vapour pressure of Liquid- Liquid solution → \rightarrow → Example → \rightarrow → Vapour pressure of solution of solid in liquid → \rightarrow → Ideal Solution & Non-Ideal Solution → \rightarrow → Azeotropes
Solutions Lecture-1
Example
P V = n R T PV=nRT P V = n RT
P A V = n A R T P_AV=n_ART P A V = n A RT
X A = n A n A + n B = P A P A + P B X_A=\frac {n_A} {n_A + n_B} = \frac {P_A} {P_A + P_B} X A = n A + n B n A = P A + P B P A
0.179 = 62.4 347.9 = 0.179 0.179= \frac {62.4} {347.9} = 0.179 0.179 = 347.9 62.4 = 0.179
X B = 0.821 X_B = 0.821 X B = 0.821
Concept of solubility → \rightarrow → Exothermic & Endothermic reaction → \rightarrow → Vapour pressure of Liquid- Liquid solution → \rightarrow → Example → \rightarrow → Vapour pressure of solution of solid in liquid → \rightarrow → Ideal Solution & Non-Ideal Solution → \rightarrow → Azeotropes
Solutions Lecture-1
Example
Vapour pressure of pure liquid A and B are 450mmHg and 700mmHg.If P T = 600 m m H g P_T=600mmHg P T = 600 mm H g find out the composition of liquid mixture.Also find out the composition of vapour phase
Solution
Concept of solubility → \rightarrow → Exothermic & Endothermic reaction → \rightarrow → Vapour pressure of Liquid- Liquid solution → \rightarrow → Example → \rightarrow → Vapour pressure of solution of solid in liquid → \rightarrow → Ideal Solution & Non-Ideal Solution → \rightarrow → Azeotropes
Solutions Lecture-1
Example
P T = P A + P B P_T=P_A+P_B P T = P A + P B
P T = 600 m m H g = 450 X A + 700 ( 1 − X A ) P_T=600 mmHg=450X_A+700(1-X_A) P T = 600 mm H g = 450 X A + 700 ( 1 − X A )
600 = 450 X A + 700 − 700 X A 600=450X_A+700-700X_A 600 = 450 X A + 700 − 700 X A
600 = 700 − 250 X A 600=700-250X_A 600 = 700 − 250 X A
Concept of solubility → \rightarrow → Exothermic & Endothermic reaction → \rightarrow → Vapour pressure of Liquid- Liquid solution → \rightarrow → Example → \rightarrow → Vapour pressure of solution of solid in liquid → \rightarrow → Ideal Solution & Non-Ideal Solution → \rightarrow → Azeotropes
Solutions Lecture-1
Example
X A = 100 250 = 0.4 X_A=\frac {100} {250}=0.4 X A = 250 100 = 0.4
X B = 1 − 0.4 = 0.6 X_B= 1-0.4=0.6 X B = 1 − 0.4 = 0.6
P A = 450 × 0.4 = 180 P_A= 450\times 0.4=180 P A = 450 × 0.4 = 180
P B = 700 × 0.6 = 420 P_B= 700\times 0.6=420 P B = 700 × 0.6 = 420
X A V = P A P T X^V_A=\frac {P_A} {P_T} X A V = P T P A
= 180 600 = 0.3 =\frac {180} {600}=0.3 = 600 180 = 0.3
X B V = 420 600 = 0.7 X^V_B=\frac {420} {600}=0.7 X B V = 600 420 = 0.7
Concept of solubility → \rightarrow → Exothermic & Endothermic reaction → \rightarrow → Vapour pressure of Liquid- Liquid solution → \rightarrow → Example → \rightarrow → Vapour pressure of solution of solid in liquid → \rightarrow → Ideal Solution & Non-Ideal Solution → \rightarrow → Azeotropes
Solutions Lecture-1
Vapour pressure of solution of solid in liquid
Concept of solubility → \rightarrow → Exothermic & Endothermic reaction → \rightarrow → Vapour pressure of Liquid- Liquid solution → \rightarrow → Example → \rightarrow → Vapour pressure of solution of solid in liquid → \rightarrow → Ideal Solution & Non-Ideal Solution → \rightarrow → Azeotropes
Solutions Lecture-1
Ideal Solution & Non-Ideal Solution
1 L of Solvent A + 2 L of Solvent B → \rightarrow → 3 L of Solution
Concept of solubility → \rightarrow → Exothermic & Endothermic reaction → \rightarrow → Vapour pressure of Liquid- Liquid solution → \rightarrow → Example → \rightarrow → Vapour pressure of solution of solid in liquid → \rightarrow → Ideal Solution & Non-Ideal Solution → \rightarrow → Azeotropes
Solutions Lecture-1
Azeotropes
Richer in more volatile component
Same concentration of liquid phase & vapour phase
Weaker interaction
Positive deviation
Minimum boiling
Negative deviation
Maximum boiling 68 68 68 %H N O 3 + H 2 O HNO_3+H_2O H N O 3 + H 2 O
Concept of solubility → \rightarrow → Exothermic & Endothermic reaction → \rightarrow → Vapour pressure of Liquid- Liquid solution → \rightarrow → Example → \rightarrow → Vapour pressure of solution of solid in liquid → \rightarrow → Ideal Solution & Non-Ideal Solution → \rightarrow → Azeotropes